Sodium hydroxide Essays

USES OF SODIUM HYDROXIDE, BLEACHING POWDER, BAKING POWDER, WASHING SODA Objective: To understand the use of common salt (NaCl) for preparation of chemicals such as Sodium hydroxide, Bleaching powder, Baking powder, Washing soda. The common salt (Chemical formula-NaCl, Chemical name- Sodium chloride) that we eat in our daily diet is the raw material for preparation of chemical compounds such as Sodium hydroxide, Bleaching powder, Baking powder, Washing soda. NaCl is a neutral salt. Sodium hydroxide

concentration of acid, we can use a known concentration of hydroxide base. This type of reaction is a neutralization reaction, where salt and water are products of the reaction: Acid + Base Salt +

acid with either sodium hydroxide (NaOH) or aqueous ammonia (NH₃). Can you make any correlation between the quantities of the heat given off and the fact that sodium hydroxide is a stronger base than ammonia (NH₃)? A negative ΔH indicates a process giving off heat, making it exothermic. Using the values collected throughout the experiment, there seems to be a trend between sodium hydroxide and aqueous ammonia, being that more heat is given off when the acids react with sodium hydroxide. From this we

Abstract The purpose of the experiment was to test which antacid medicine was most effective in decreasing the acidity levels in the stomach. Titration experiments involving hydrochloric acid and sodium hydroxide were used to test different antacids to see which one needed the least amount of sodium hydroxide to turn the solution pink. The antacids that were being compared in this experiment were Alcalak, Alka-Seltzer and Medi-First. With the use of M1 x V1 = M2 x V2 the excess volume of hydrochloric

triprotic acid, with different volumes of sodium hydroxide. Introduction Procedure Phosphoric acid solution with a volume of 1.00 mL and a molarity of 6.00 M was transferred into a 125-mL Erlenmeyer flask using a volumetric pipette. Sodium hydroxide solution with a volume of 6.00 mL and a molarity of 3.00 M was transferred into a 50 mL beaker using a volumetric pipette. While swirling the phosphoric acid solution in the Erlenmeyer flask, the sodium hydroxide solution was added to it a few drops at

the obtained knowledge of the total acidity, the experiment can be performed with the purpose of determining the amount of %w/w of citric acid in Kool-Aid. Using a titrimetric analysis method, the analyte, total solution acidity and titrant, sodium hydroxide, undergo an acid-base titration. Differing from the redox titration undergone in experiment two in which the ascorbic acid is reacted with the reduced iodate in the presence of iodine ion generating iodine, which is the form that is used to further

acid was poured into the flask until there was a permanent pink colour. The acid was allowed to be poured for a little longer before the flask was removed and taken to a lab bench with a buret that contained 0.1 M sodium hydroxide, and the amount of acid used was recorded. The sodium hydroxide was added into the flask in small amounts

calcium chloride with 2 mL sodium phosphate, adding a few drops of water to a test tube containing 0.5 g copper sulfate, heating 0.5 g of copper(II) hydroxide in a test tube, adding a square piece of zinc to a test tube containing 3 mL 3M hydrochloric acid, mixing 2 mL 3M hydrochloric acid with 2 mL sodium carbonate, adding 0.1 g MnO2 to a test tube with 3 mL hydrogen peroxide, combusting a sodium acetate and ethanol solution, mixing 3 g ammonium chloride and 7 g strontium hydroxide octahydrate together

KHC8H4O4 in order to determine the molar concentration of the NaOH solution. As seen in Table 1, the known mass of KHC8H4O4 was 0.2037 g. The moles of KHC8H4O4, could then be calculated to get 9.97E-04 mol. Based on the balanced equation between the sodium hydroxide solution and primary standard acid, the mole ratio of 1:1 and the molar mass of NaOH was applied to calculate the molar concentration of NaOH, which was 5.42E-02 mol/L (Table 2). Since there was only one trial conducted for this part, the average

Beginning with the principles, Brønsted-Lowry acid base theory demonstrates that an acid donates a hydrogen ions, while a base accepts hydrogen ions. Strong acids have the an easier ability to donate hydrogen ions compared to weak acids.The goal for Experiment 8 Acid-Base Equilibria: Determination of Acid Ionization Constants is to recognize how different amounts of quantitative values can alter the pH in a solution. This procedure was carried out by mixinging specific acid or base solutions together

Determining the percentage of sodium carbonate in a sample of washing soda crystals Aim The purpose of the experiment carried out was to determine the percentage of sodium carbonate (Na2CO3) in a known amount of washing soda crystal, using the titration technique. Acids & Bases Water is the most common acid and base found on earth. An acid is anything that can donate a proton/H+ and a base is anything that can accept a proton/H+ – Bronsted-Lowry. Water being able to both accept and donate a proton/H+

benzoic) to ions. Hydroxide ions on the other hand convert Phenols to ions. This makes them soluble in the aqueous layer as ions are soluble in water. However, addition of HCl to the aqueous ionic solutions regenerates non-ionic substances which are only soluble in the organic layer. Materials • 2M diethyl ether • Saturated NaCl solution • Saturated aqueous solution of Sodium bicarbonate

which has to deal with the laws according to which substances unite to form chemical compounds." In this exercise, we combined copper(II) sulfate pentahydrate with two moles of sodium hydroxide which produced copper(II) hydroxide and sodium sulfate (CuSO4 + 5H2O +2NaOH  Cu(OH)2 + Na2SO4). We then dissociated copper(II) hydroxide to produce copper(II) oxide and water (Cu(OH)2  CuO + H2O). The objective of this exercise is to perform a simple chemical reaction where the concept of stoichiometry is put

Purpose: The purpose of this lab is to titrate an unknown solid acid (KH2PO4) with a standardized sodium hydroxide solution. After recording and plotting the data, the acid’s equivalence point will be recorded once the color changes. Using the equivalence point, the halfway point will be calculated, which is used to determine the acid’s equilibrium constant. The acid’s calculated equilibrium constant will be compared with the acid’s established pKa value. Eventually using the NaOH and the acid’s

experiment, citric acid was titrated with sodium hydroxide producing an endpoint between pH range of 8.3-10. (EASYCHEM, 2018) Citric acid has three acidic protons therefore it is a triprotic acid (lumen, 2018). The accurate concentration of the sodium hydroxide must be known to determine the citric acid concentration. The aim of this experiment was to determine the citric acid(weak acid) content of Lemon Juice by titrating it with standard sodium hydroxide solution(strong base). Commercially available

becomes high enough to cause discomfort, brought about by the ingestion of certain types of food, an antacid preparation can be taken to neutralize the excess stomach acid. The active ingredient in every antacid is a base, the most common being metal hydroxides, metal carbonates or a mixture of the two. Table 1 lists the active ingredients in several commercial brands of antacid. Table 1. Brands of antacid tablets and their major ingredients Brand Name Major ingredient Recommended dose Alka-Seltzer NaHCO3

The experiment for this report is 5, 6, and 7. In experiment 5 there are given a Sodium Hydroxide which is 4.126 g when it is weighted and a KHP also with the NaOH there’s two other experiment that are used to find the titration of molarity in the three chemical balances. In exp. 6 and 7 there using the NaOH to find titration in an acid and vinegar by going through three trails to see how much sodium hydroxide is pick in it until it turns light pink, however if it turns dark pink there’s an error

of a given material known as concentration is in a substance or mixture. In this lab, the student also learns the technique of using titration. The concentration of the acid we used in class will be sampled with a standardize solution such as sodium hydroxide with an environmentally indicator to show the physical change of color that occurs to the solution by the acid. The equipment necessary for the titration experiment follows: 0.1M NaOH, Acid solution, Anthocyanin (which is found in red cabbage

evaporator, obtaining crude trimyristin, which was then purified via recrystallization with 95% ethanol. This yielded 0.230g of purified trimyristin, in the form of a white powder. The trimyristin was then mixed with sodium hydroxide and 95% ethanol under gentle reflux, yielding sodium myristate. Finally, concentrated hydrochloric acid was added dropwise, yielding myristic acid. I obtained a yield of 408.3% (0.523g) of the myristic acid

In the chemical reaction of hydrochloric acid, HCl, and sodium hydroxide, NaOH, the theoretical ratio is one HCL for every one NaOH. By then taking a known measurement of HCl, in this case 10mL, in addition to the phenolphthalein indicator and deionized water, and titrating it with NaOH, the amount of NaOH that causes the reaction to be complete was calculable given that we know when the reaction was complete. After calculating the moles of each substance added to complete the reaction, the experimental